Volumetric and Viscometric Properties of Binary Liquid Mixtures of

Mar 5, 2010 - Department of Chemistry, Kurukshetra University, Kurukshetra 136 119, India. J. Chem. Eng. Data , 2010, 55 (4), pp 1700–1703. DOI: 10...
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J. Chem. Eng. Data 2010, 55, 1700–1703

Volumetric and Viscometric Properties of Binary Liquid Mixtures of Ethylene Glycol Monomethyl Ether + 1-Hexanol, 1-Octanol, and 1-Decanol at Temperatures of T ) (293.15, 298.15, 303.15, and 308.15) K Gyan Prakash Dubey* and Krishan Kumar† Department of Chemistry, Kurukshetra University, Kurukshetra 136 119, India

Density, viscosity, and speed of sound have been measured for the binary mixtures of ethylene glycol monomethyl ether (CH3OCH2CH2OH) with 1-hexanol (C6H14O), 1-octanol (C8H18O), and 1-decanol (C10H22O) at temperatures of T ) (293.15, 298.15, 303.15, and 308.15) K and at a pressure of 0.1 MPa as a function of composition. The experimental density, F, values were used to calculate the excess molar volumes, VEm. The isentropic compressibilities, κS, have also been calculated with experimental densities and speeds of sound data. The values of VEm were fitted to the Redlich-Kister polynomial equation and have been used to discuss the presence of significant interactions between polyether and alcohol molecules.

Introduction

Experimental Section

Glycol ethers are important industrial solvents. They can be used as scrubbing liquids for the absorption of acid gases in the cleaning of exhaust air and gas streams from industrial production plants because of their favorable properties such as low vapor pressure, low toxicity, low viscosity, high chemical stability, and low melting temperature.1 In last years, some authors have proposed new organic working pairs containing ethylene glycol ethers as absorbent fluids for absorption heat pumps and chillers.2,3 In addition, the glycol ethers can also be used as polar additives in anionic polymerization and automotive brake fluid. Ethylene glycol monomethyl ether (EGMME, 2-methoxyethanol) is a colorless liquid which is miscible with alcohols and most organic solvents. It is widely used as solvents, especially in the printing ink and paint industries. Systematic studies of the thermodynamic excess properties of ether and alcohol mixtures are important from the viewpoint of understanding the molecular liquid structure and the intermolecular interactions dominated by the self-association of alcohols due to hydrogen bonding. Alcohols are the well-known solvents with protic and self-associated properties, which are used to study the hydrophobic effects. Ethers and 1-alkanols are used in the chemical industry as a solvent for oils and petrol and are used in gasoline formulation as an enhancement of octane rating or fuel additives. The present work concerns the experimental measurements of densities, F, viscosities, η, and speed of sound, u, for binary mixtures of EGMME with 1-hexanol, 1-octanol, and 1-decanol at temperatures of T ) (293.15, 298.15, 303.15, and 308.15) K and at atmospheric pressure. Furthermore, using experimental results, excess molar volumes, VEm, have been determined to gain a better understanding of the intermolecular interactions between the mixing components. * To whom correspondence should be addressed. E-mail: gyan.dubey@ rediffmail.com. † E-mail: [email protected].

Materials. EGMME (CAS Registry No.: 109-86-4 with a mass fraction purity of 0.995), 1-hexanol (mass fraction purity of 0.985), 1-octanol (mass fraction purity of 0.995), and 1-decanol (mass fraction purity of 0.995) were obtained from S. D. Fine Chemicals Ltd. All of the chemicals were partially degassed before use. The experimentally measured values of densities, viscosities, and speeds of sound of all of the pure components at T ) 298.15 K are compared with literature4-13 and are presented in Table 1. Apparatus and Procedure. The EGMME + alcohol binary mixture can be prepared by weighing appropriate amounts of EGMME and alcohol on an Afcoset-ER-120A electronic balance, with a precision of ( 0.05 mg, by syringing each component into airtight stoppered bottles to minimize evaporation losses. The pure components were separately degassed by vacuum pump shortly before sample preparation. The accuracy of mole fractions was ( 1 · 10-4. Density, F, and speed of sound, u, were measured by using a digital vibrating tube density and speed of sound analyzer (Anton Paar DSA 5000), having two integrated Pt 100 thermometers with a proportional temperature controller that kept the sample at the required temperature. The apparatus was calibrated at working temperatures with dry air, double toluene,10,12 cyclohexane,10,13 and distilled water.14 The temperature in the cell was regulated to ( 0.001 K with an in-built solid state thermostat by the Peltier method. The uncertainty in the density measurement is ( 2 · 10-3 kg · m-3 and for the speed of sound ( 0.1 m · s-1. To perform the measurement, one out of a total of 10 individual measuring methods was selected, and the measuring cell was filled with the sample. An acoustic signal informed us when the measurement was completed. The results are automatically converted (including temperature compensation wherever necessary) into concentration, specific gravity, or other density-related units using the built-in conversion tables and functions. The kinematic viscosities ν () η/F) of pure liquids and liquid mixtures were measured at T ) 298.15 K and at atmospheric pressure using an Ubbelohde suspended-level viscometer. The

10.1021/je9005344  2010 American Chemical Society Published on Web 03/05/2010

Journal of Chemical & Engineering Data, Vol. 55, No. 4, 2010 1701 Table 1. Experimental and Literature Values of Densities (G*), Viscosities (η*), and Speeds of Sound (u*) of Pure Liquid Components at T/K ) 298.15 F* · 10-3/kg · m-3

u*/m · s-1

η*/mPa · s

components

exptl

lit.

exptl

lit.

exptl

lit.

C6H14O C8H18O C10H22O CH3OCH2CH2OH C6H6 C6H12 C7H8

0.815265 0.821794 0.826470 0.960978 0.873710 0.773790 0.862194

0.8155334 0.8211816 0.8266409 0.96024010 0.8737012 0.7738910 0.8621910

4.439 7.143 11.192 1.512 0.604 0.902 0.556

4.5945 7.4987 11.7357 1.54111 0.60412 0.89812 0.55612

1303.2 1347.6 1379.9 1343.5 1299.1 1253.3 1304.7

1304.725 1348.008 1380.015 1343.4510 1299.212 1253.213 1304.312

viscometer was calibrated so as to determine the two constants C1 and C2 in the equation η/F ) C1t - C2/t, obtained by measuring the flow time t with double-distilled water10 and cyclohexane.12 The viscometer is filled with liquid or liquid mixtures, and its limbs were closed with Teflon caps, taking due precautions to minimize the evaporation losses. The flow time measurements were made by using an electronic stopwatch with a precision of ( 0.1 s. An average of four or five sets of flow times for each liquid or liquid mixture was taken for calculating the viscosity. The measured values of kinematic viscosities were converted to dynamic viscosities after multiplication by the density. The uncertainty in the viscosity measurements, based on our work on several pure liquids, was ( 0.003 mPa · s. In viscosity measurements, the temperature of the samples was controlled by using a water bath equipped with a thermostat with an accuracy of ( 0.01 K. The uncertainties in density, viscosity, and speed of sound are determined by comparing the experimental values of standard liquids with their literature values at that temperature.

Figure 1. Excess molar volumes against mole fractions x1CH3 at T ) 298.15 K. 9, (OCH2CH2OH + C6H14O); b, (OCH2CH2OH + C8H18O); 2, (OCH2CH2OH + C10H22O); 1, ref 16. The solid curves have been derived from the Redlich-Kister eq 2.

Results and Discussion E Density, F, speed of sound, u, excess molar volume, Vm , and isentropic compressibility, κS, determined by means of the Laplace equation (κS ) F-1u-2), and viscosity, η, at temperatures of T ) (293.15, 298.15, 303.15, and 308.15) K and p ) 0.1 MPa for (CH3OCH2CH2OH + C6H14O, + C8H18O, or + C10H22O) are reported in Table 2. Excess molar volumes, deviation in speeds of sound, and deviation in isentropic compressibilities were derived respectively from the expressions

2

E Vm )

∑ xiMi(F-1 - Fi-1)

(1)

i)1

where Fi is the density of the pure components, F is the density of the mixtures, and xi is the mole fraction. The viscosity deviations are calculated from their linear dependence by using the following relation. The experimental results were fitted in the Redlich-Kister polynomial equation15 p

Y(x) ) x1x2

∑ Ai(x1 - x2)i

(2)

i)1

where p is the number of estimated parameters of Ai. The standard deviation was calculated using the relation: n

σ)[

∑ {Y(x)exptl - Y(x)cal}2/n]1/2

(3)

i)1

where Y(x)exptl and Y(x)cal are the values of the experimental E ), respectively, and n is the and calculated properties (F, η, Vm

number of experimental data points. The calculated values of the coefficients (Ai) along with standard deviations (σ) are reported in Table 3. Figure 1 shows that excess molar volumes are positive over the entire range of composition increasing magnitude with the increase in number of carbon atom in alcohol molecules. The E is obtained for the maximum positive value of Vm CH3OCH2CH2OH + C10H22O mixture. It indicates that interaction between EGMME and alcohol molecules is weak. This kind of interaction is also affected by temperature and composition. The interaction becomes weaker with increasing the temperature E with the rise in as suggested by increasing values of Vm temperature. The positive value of VEm can be visualized as being due to a closer approach of the unlike molecules having significantly different molecular sizes. Because of mixing, the already existing self-association of ether and alcohol molecules breaks, and the system shows weak intermolecular interactions. The longer the chain length of the alcohol molecules, the weaker the interaction between liquid components will be. To the best of our knowledge, no data in literature are available for a comparison of the excess molar volume values of the studied systems at T ) 298.15 K. However, a comparison has been made with the values reported by Ramana Reddy et al.16 for the binary mixtures of 2-ethoxyethanol (an alkoxy alkanol of the series of EGMME) + pentanol at T ) 308.15 K that support our results. For the comparison, the data points of excess molar volume of 2-ethoxyethanol + pentanol at T ) 308.15 K have been shown in Figure 1.

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Journal of Chemical & Engineering Data, Vol. 55, No. 4, 2010

E Table 2. Densities (G), Excess Molar Volumes (Vm ), Speeds of Sound (u), Isentropic Compressibilities (KS), and Viscosity (η) for Binary Mixtures from T ) (293.15 to 308.15) K

F · 10-3

E Vm · 106

u

κS

η

m3 · mol-1

m · s-1

TPa-1

mPa · s

0.0516 0.0979 0.1486 0.2049 0.2500 0.2987 0.4088 0.5134 0.5991 0.6915 0.8050 0.9039

x1CH3OCH2CH2OH + x2C6H14O 0.823245 0.0700 1319.2 698.01 0.827405 0.1233 1318.4 695.31 0.832198 0.1718 1317.7 692.01 0.837755 0.2238 1317.3 687.84 0.842351 0.2702 1316.9 684.55 0.847639 0.3035 1316.3 680.85 0.860712 0.3363 1317.3 677.02 0.874132 0.3918 1318.6 657.96 0.886614 0.3814 1321.2 646.17 0.901590 0.3351 1325.9 630.93 0.922045 0.2715 1334.2 609.27 0.942547 0.1665 1345.0 586.45

4.203 4.000 3.764 3.486 3.257 3.122 2.675 2.438 2.250 2.092 1.858 1.737

0.0535 0.1073 0.1407 0.2002 0.2659 0.2973 0.3559 0.5233 0.6059 0.7126 0.7903 0.9202

x1CH3OCH2CH2OH + x2C8H18O 0.828636 0.0885 1362.0 650.55 0.832242 0.1723 1359.3 650.33 0.834668 0.2100 1357.9 650.00 0.839135 0.2899 1354.9 649.17 0.844444 0.3736 1351.9 647.99 0.847294 0.3865 1350.5 647.07 0.852613 0.4547 1348.0 645.46 0.870970 0.5311 1342.3 637.26 0.881954 0.5291 1340.4 631.12 0.898662 0.4767 1339.7 620.03 0.912569 0.4513 1340.9 609.42 0.942675 0.1950 1349.3 582.62

7.447 6.742 6.355 5.659 4.991 4.779 4.259 3.272 2.863 2.432 2.150 1.772

0.0606 0.1173 0.1631 0.1934 0.2510 0.3025 0.4130 0.5170 0.6285 0.7087 0.7965 0.9382

x1CH3OCH2CH2OH + x2C10H22O 0.832950 0.1006 1393.1 618.63 0.835952 0.2112 1389.5 619.58 0.838564 0.2943 1386.6 620.24 0.840414 0.3420 1384.7 620.56 0.844262 0.4092 1380.8 621.26 0.847887 0.4840 1377.5 621.54 0.856970 0.5860 1370.2 621.54 0.867321 0.6390 1363.6 620.08 0.880912 0.6557 1356.6 616.81 0.892252 0.6180 1352.5 612.23 0.909015 0.5267 1349.5 604.07 0.944534 0.2161 1352.5 578.78

11.479 10.191 9.351 8.764 7.828 7.137 5.850 4.593 3.746 3.119 2.574 1.840

x1

-3

kg · m

T/K ) 293.15

T/K ) 298.15 0.0516 0.0979 0.1486 0.2049 0.2500 0.2987 0.4088 0.5134 0.5991 0.6915 0.8050 0.9039

x1CH3OCH2CH2OH + x2C6H14O 0.819629 0.0717 1302.2 719.44 0.823749 0.1270 1301.5 716.72 0.828504 0.1763 1300.8 713.25 0.834013 0.2299 1300.5 708.98 0.838571 0.2772 1300.0 705.57 0.843810 0.3123 1299.4 701.84 0.856785 0.3459 1300.5 697.98 0.870100 0.4027 1301.6 678.32 0.882495 0.3919 1304.2 666.14 0.897370 0.3445 1308.8 650.50 0.917699 0.2784 1317.1 628.14 0.938079 0.1705 1327.8 604.58

3.788 3.612 3.329 3.101 2.955 2.775 2.435 2.207 2.038 1.890 1.706 1.602

0.0535 0.1073 0.1407 0.2002 0.2659 0.2973 0.3559 0.5233 0.6059 0.7126 0.7903 0.9202

x1CH3OCH2CH2OH + x2C8H18O 0.825138 0.0903 1345.0 669.90 0.828704 0.1765 1342.3 669.70 0.831104 0.2165 1340.6 669.44 0.835528 0.2968 1337.9 668.62 0.840786 0.3821 1334.9 667.45 0.843606 0.3961 1333.6 666.54 0.848877 0.4655 1331.1 664.91 0.870970 0.5435 1325.3 656.64 0.867068 0.5412 1323.4 650.30 0.877961 0.4886 1322.6 639.08 0.908335 0.4607 1323.9 628.13 0.938234 0.1991 1332.1 600.59

6.475 5.801 5.490 5.141 4.428 4.200 3.239 2.919 2.583 2.204 1.965 1.631

Table 2a. Continued F · 10-3

E Vm · 106

u

κS

η

kg · m-3

m3 · mol-1

m · s-1

TPa-1

mPa · s

0.0606 0.1173 0.1631 0.1934 0.2510 0.3025 0.4130 0.5170 0.6285 0.7087 0.7965 0.9382

x1CH3OCH2CH2OH + x2C10H22O 0.829505 0.1023 1375.9 636.78 0.832457 0.2152 1372.4 637.81 0.835060 0.2987 1369.5 638.46 0.836878 0.3497 1367.5 638.95 0.840695 0.4165 1363.7 639.58 0.844280 0.4930 1360.4 639.96 0.853268 0.5975 1353.1 640.10 0.863518 0.6518 1346.5 638.47 0.876980 0.6690 1339.6 635.45 0.888913 0.6306 1335.3 630.88 0.904836 0.5379 1332.3 622.64 0.940097 0.2195 1335.3 596.54

9.653 8.800 8.019 7.552 6.856 6.099 4.133 4.090 3.310 2.807 2.332 1.693

0.0516 0.0979 0.1486 0.2049 0.2500 0.2987 0.4088 0.5134 0.5991 0.6915 0.8050 0.9039

x1CH3OCH2CH2OH + x2C6H14O 0.815993 0.0724 1285.5 741.54 0.820074 0.1295 1284.7 738.79 0.824786 0.1806 1284.1 735.28 0.830247 0.2357 1283.7 730.91 0.834763 0.2846 1283.3 727.42 0.839961 0.3204 1282.7 723.59 0.852828 0.3562 1283.6 719.63 0.866048 0.4130 1284.8 699.49 0.878355 0.4020 1287.3 686.97 0.893130 0.3540 1291.9 670.83 0.913334 0.2848 1300.1 647.34 0.933591 0.1742 1310.7 623.45

3.221 3.093 2.905 2.697 2.566 2.433 2.148 1.943 1.797 1.691 1.527 1.436

0.0535 0.1073 0.1407 0.2002 0.2659 0.2973 0.3559 0.5233 0.6059 0.7126 0.7903 0.9202

x1CH3OCH2CH2OH + x2C8H14O 0.821625 0.0911 1328.2 690.192 0.825153 0.1794 1325.5 689.762 0.827528 0.2195 1323.9 689.498 0.831905 0.3029 1321.1 688.708 0.837111 0.3899 1318.1 687.564 0.839904 0.4047 1316.8 686.673 0.845122 0.4752 1314.2 685.064 0.863148 0.5555 1308.5 676.696 0.873942 0.5540 1306.5 670.345 0.890382 0.4920 1305.7 658.774 0.904076 0.4706 1306.9 647.615 0.933772 0.2029 1315.0 619.290

5.399 4.894 4.663 4.281 3.776 3.588 3.209 2.543 2.274 1.950 1.753 1.470

0.0606 0.1173 0.1631 0.1934 0.2510 0.3025 0.4130 0.5170 0.6285 0.7087 0.7965 0.9382

x1CH3OCH2CH2OH + x2C10H22O 0.826050 0.1045 1358.9 655.49 0.828982 0.2194 1355.4 656.65 0.831539 0.3049 1352.5 657.36 0.833342 0.3558 1350.6 657.82 0.837111 0.4255 1346.8 658.58 0.840662 0.5023 1343.5 658.99 0.849553 0.6097 1336.2 659.27 0.859697 0.6657 1329.6 658.00 0.873028 0.6834 1322.6 654.83 0.884854 0.6440 1318.4 650.20 0.900644 0.5489 1315.3 641.83 0.935630 0.2039 1318.15 615.13

7.925 7.221 6.275 5.685 5.154 4.243 3.514 2.870 2.471 2.055 1.527 1.470

0.0516 0.0979 0.1486 0.2049 0.2500 0.2987 0.4088 0.5134 0.5991 0.6915 0.8050 0.9039

x1CH3OCH2CH2OH + x2C6H14O 0.812325 0.0749 1268.9 764.50 0.816370 0.1333 1267.2 761.65 0.821037 0.1864 1267.5 758.17 0.826451 0.2430 1267.0 753.69 0.830930 0.2927 1266.6 750.13 0.836084 0.3295 1206.0 822.31 0.848853 0.3662 1266.9 733.91 0.861965 0.4245 1268.0 721.49 0.874185 0.4130 1270.6 708.61 0.888857 0.3638 1275.0 692.02 0.908936 0.2923 1283.2 668.17 0.929076 0.1781 1293.7 643.12

x1

T/K ) 303.15

T/K ) 308.15 2.748 2.661 2.504 2.369 2.218 2.107 1.958 1.754 1.572 1.494 1.364 1.276

Journal of Chemical & Engineering Data, Vol. 55, No. 4, 2010 1703 Table 2b. Continued F · 10 x1

-3

kg · m-3

E Vm · 106

u

κS

η

m3 · mol-1

m · s-1

TPa-1

mPa · s

0.0535 0.1073 0.1407 0.2002 0.2659 0.2973 0.3559 0.5233 0.6059 0.7126 0.7903 0.9202

x1CH3OCH2CH2OH + x2C8H18O 0.818089 0.0937 1311.5 0.821583 0.1832 1308.9 0.823931 0.2248 1307.2 0.828261 0.3104 1304.4 0.833414 0.3922 1301.4 0.836178 0.4148 1300.1 0.841346 0.4864 1297.5 0.859203 0.5688 1296.5 0.869902 0.5673 1289.7 0.886205 0.5114 1288.8 0.899757 0.4848 1290.0 0.929291 0.2052 1298.0

710.63 710.46 710.30 709.54 708.44 707.55 705.97 697.57 691.14 679.37 667.88 638.75

4.496 4.118 3.921 3.537 3.258 3.181 2.817 2.217 1.990 1.751 1.436 1.343

0.0606 0.1173 0.1631 0.1934 0.2510 0.3025 0.4130 0.5170 0.6285 0.7087 0.7965 0.9382

x1CH3OCH2CH2OH + x2C10H22O 0.822580 0.1058 1342.2 674.86 0.825482 0.2218 1338.6 676.03 0.828008 0.3093 1335.8 676.85 0.829786 0.3621 1333.8 677.40 0.833512 0.4337 1330.0 678.27 0.837024 0.5119 1326.7 678.74 0.845819 0.6218 1319.4 679.17 0.855861 0.6789 1312.8 677.98 0.869056 0.6978 1305.7 674.94 0.880773 0.6576 1301.5 670.31 0.896427 0.5603 1298.3 661.80 0.931137 0.2284 1301.1 634.42

6.627 5.998 5.540 5.261 4.794 4.383 3.672 3.051 2.491 2.154 1.537 1.350

Table 3. Coefficients Ai of the Redlich-Kister Equation 2 along with Standard Deviations (σ) for Binary Mixtures at T ) (293.15 to E 308.15) K for Excess Molar Volume (Vm ) T/K

A0

A1

A2

A3

A4

σ

293.15 298.15 303.15 308.15

1.4796 1.5465 1.5892 1.6359

x1CH3OCH2CH2OH + x2C6H14O 0.2742 0.2324 0.2804 0.1615 0.2857 0.1500 0.2778 0.1257

293.15 298.15 303.15 308.15

2.2584 2.1465 2.1918 2.2462

x1CH3OCH2CH2OH + x2C8H18O 0.7256 -0.0473 0.6363 0.2868 0.6404 0.2701 0.6790 0.2852

0.0305 0.0149 0.0165 0.0622

293.15 298.15 303.15 308.15

2.5361 2.5860 2.6407 2.6940

x1CH3OCH2CH2OH + x2C10H22O 0.8210 0.6604 0.2715 -0.4220 0.8459 0.6835 0.2622 -0.4574 0.8702 0.6869 0.2549 -0.4575 0.8922 0.7059 0.2708 -0.495

0.0069 0.0072 0.0070 0.0070

0.0089 0.0111 0.011 0.0107

Conclusions In this paper, an attempt is made to measure densities, viscosities, and speed of sound at T ) (293.15, 298.15, 303.15, and 308.15) K over the entire range of mixture composition of EGMME with 1-hexanol, 1-octanol, and 1-decanol. Out of these measured data, the excess molar volumes have been calculated and correlated by a Redlich-Kister type polynomial equation to derive the coefficients and standard deviations.

E for all Positive deviations are observed in the case of Vm binary mixtures. On the whole it can be concluded that the strength of bonding is expected to decrease with an increase in the chain length of alcohols as well as with rise of temperature. E corroborate this fact. The present results of Vm

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Received for review June 26, 2009. Accepted February 21, 2010.

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